The following diagram represents the reaction of (red spheres) with (blue spheres):

How many moles of product can be made from 1.0 mol of A2? From 1.0 mol of B2?

Verified step by step guidance

1. Identify the reactants and products in the reaction: X2 (red spheres) and Y2 (blue spheres) react to form XY3.
2. Write the balanced chemical equation for the reaction: X2 + 3Y2 -> 2XY3.
3. Determine the mole ratio from the balanced equation: 1 mole of X2 reacts with 3 moles of Y2 to produce 2 moles of XY3.
4. Calculate the moles of product from 1.0 mol of X2: Use the mole ratio to find how many moles of XY3 can be formed.
5. Calculate the moles of product from 1.0 mol of Y2: Use the mole ratio to find how many moles of XY3 can be formed.

Key Concepts

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to predict how much of each substance is consumed or produced based on balanced chemical equations. Understanding stoichiometry is essential for calculating the moles of products formed from given moles of reactants.

Mole Ratio

The mole ratio is derived from the coefficients of a balanced chemical equation and indicates the proportion of moles of one substance to another in a reaction. For example, if the reaction shows that 1 mole of A2 reacts with 2 moles of B2 to produce 1 mole of XY3, this ratio is crucial for determining how many moles of product can be formed from a specific amount of reactants.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is vital for accurate stoichiometric calculations, as it dictates how much of the product can be produced based on the initial amounts of reactants available.